Quantum Theory

Question 1

Plank

Answer 1

Different atoms and molecules can emit or absorb energy in discrete quantities only. The smallest amount of energy that can be emitted or absorbed in the form of electromagnetic radiation is known as quantum

Question 2

equation given by Planck

Answer 2

E=hν

Question 3

Planck’s constant

Answer 3

h = 6.626 x 10^-34 J s

Question 4

Einstein

Answer 4

uses Planck’s quantum theory and uses it to try and explain the photoelectric effect

Question 5

photoelectric effect

Answer 5

• if longer wavelengths deliver smaller packets, it may not be enough to move electrons from the metal
• if shorter wavelengths deliver larger packets, the packet of energy acting like a particle is enough to dislodge electrons from the metal

Question 6

Niels Bohr

Answer 6

applies Planck’s quantum theory to line spectra of elements; Bohr’s model

Question 7

Bohr’s Assumptions

Answer 7

1) electrons are particles
2) energy of the atom must be quantized
3) orbitals are fixed and circular
- labeled each level “n”
- n = 1 is the closest to the nucleus
- lowest energy state of the atom is the
ground state
4) electrons absorb energy and jump to
higher levels (excited state)

Question 8

line spectra

Answer 8

atomic emission spectrum that contains only certain wavelengths of light ( continuous spectrum = rainbow )

Question 9

ground state

Answer 9

lowest energy level fro the electrons in an atom

Question 10

excited state

Answer 10

upon the electron’s absorption of energy, there are jumps to higher levels